For each of the following processes that occur in an open steady state system, calcu- late the heat transfer to or from the system if it is isothermal. (a) 1000 g of O₂ are mixed with 1000 g of CO₂. (b) 900 kg of water are mixed with 63 kg of nitric acid. Data at SC: Compound Ĥ¦ (kJ/kg) HNO, (liquid) - 173.234 In 1 g mol H₂O -186.347 2 H₂O -193.318 5 H₂O -201.962 10 H₂O -205.014 50 H₂O -205.978 100 H₂O -205.983
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- A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = JThe specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.
- a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?A piston/cylinder setup contains 1 kg of air at 20°C with an initial volume of V1=0.1 m3, as shown in Fig. Q7. Initially, the piston rests on some stops, but it is possible for it to move within the cylinder without friction. To lift the piston and start such motion, an air pressure of 1400 kPa is required. Now, heat is transferred to the system so that the temperature of the air reaches to a final value of 300°C. Fig. Q7 A. Which statement is true? The air can lift the piston before the temperature reaches to 300°C The air cannot lift the piston before the temperature reaches to 300°C
- a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process. a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/molMeztiza, a beer cocktail, is prepared by mixing rum, beer, and cola. Compute the finalconcentration(%w/v) of ethanol in meztiza if 100.0 mL of beer was first mixed with 5.0 mL rum andbefore finally diluting it with cola to produce 200.0 mL of the beer cocktail. ( a beer contains about 4.50% (v/v) of ethanolfermented by yeast from sugars while rum contains about 40.0% (v/v) ethanol. Meanwhile, arubbing alcohol is also an alcohol solution which contains 70.0 %(v/v) isopropyl alcohol fermentedby a bacterium instead of a yeast)
- Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively Calculate the work done when 1.0 mole of nitroglycerin decomposes and additionally explain the significance of the sign.1. Calculate the standard enthalpy of formation of C10H10. Its standard enthalpy of combustion is shown by the equation: 2C10H10 (l) + 25O2 (g) → 20CO2 (g) + 10H2O (l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15oC : CO2 = -393.5 ; H2O(l) = -285.8 2. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 3. In the picture, Find the the ∆H°rxn if ∆G°rxn is 420 kJ/mol and ∆S°rxn is -143 J/mol*kA coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹